The value of the equilibrium constant (Kc) as represented by the first chemical equation is 2.70 x 10-3 at 1200 K. Calculate the value of the equilibrium constant (Kc) for the second equation at the same temperature. Express answer in scientific notation.
F2(g) = 2F(g)
2F(g) = F2(g)
Equation 1 and 2 are just the reverse of ech other. If you have K for one of them, K for the other is just the reciprocal of the first. So if k is 2.7 x 10^-3, the reverse is 1/2.70 x 10^-3.
To calculate the value of the equilibrium constant (Kc) for the second chemical equation at the same temperature, we need to use the relationship between the two equations.
The equilibrium constant (Kc) is a ratio of the concentrations of the products to the concentrations of the reactants, each raised to the power of their respective stoichiometric coefficients. In this case, the first equation is:
F2(g) ⇌ 2F(g)
The equilibrium constant (Kc1) for this equation is given as 2.70 x 10^(-3).
The second equation is:
2F(g) ⇌ F2(g)
To relate the equilibrium constants of the two equations (Kc1 and Kc2), we need to invert the first equation by taking the reciprocal of the first equilibrium constant. So, Kc1 becomes 1/Kc1:
1/Kc1 = 1/(2.70 x 10^(-3))
To calculate the value of the equilibrium constant (Kc2) for the second equation, we simply substitute the inverted value of Kc1 into the equation:
Kc2 = (1/Kc1)^(1/coefficient)
In this case, the coefficient of the product, F2(g), in the second equation is 1, so we raise the inverted Kc1 value to the power of 1:
Kc2 = (1/(2.70 x 10^(-3)))^(1/1)
Simplifying the equation:
Kc2 = 1/(2.70 x 10^(-3))
Thus, the value of the equilibrium constant (Kc2) for the second chemical equation at the given temperature is also 1/(2.70 x 10^(-3)) in scientific notation.